Probing the Orbital Energy of an Electron in an AtomJames L. BillsThis article answers an appeal for simple theoretical interpretations of atomic properties. A theoretical snapshot of an atom, showing the screened nuclear charge and the electron to be ionized at its radius of zero kinetic energy, enables anyone to approximate its ionization energy.Bills, James L. J. Chem. Educ.2006, 83, 473.

Atomic Properties / Structure |

Main-Group Elements |

Periodicity / Periodic Table |

Physical Properties |

Quantum Chemistry |

Theoretical Chemistry

Trends in Ionization Energy of Transition-Metal ElementsPaul S. MatsumotoExamines why, as the number of protons increase along a row in the periodic table, the first ionization energies of the transition-metal elements are relatively steady, but that for the main-group elements increases.Matsumoto, Paul S. J. Chem. Educ.2005, 82, 1660.

Atomic Properties / Structure |

Periodicity / Periodic Table |

Transition Elements

A Program of Computational Chemistry Exercises for the First-Semester General Chemistry CourseScott E. Feller, Richard F. Dallinger, and Paul Caylor McKinneyA series of 13 molecular modeling exercises designed for the first-semester general chemistry course is described. The modeling exercises, which are used as both prelecture explorations and postlecture problems, increase in difficulty and in student independence.Feller, Scott E.; Dallinger, Richard F.; McKinney, Paul Caylor. J. Chem. Educ.2004, 81, 283.

Ionization Energies, Parallel Spins, and the Stability of Half-Filled ShellsPeter CannThree methods for explaining the decrease in first ionization energies between group V and group VI elements are described and commented upon. The quantum mechanical origin of the unhelpful concept of half-shell stability is explained in terms of exchange energy, for which the alternative term parallel spin avoidance factor is suggested. It is recommended that for pre-university students the simplest explanation, in terms of Coulombic repulsion between two electrons occupying the same orbital, is adopted: it involves fewer difficult concepts than the other explanations and its predictions are no less accurate. Cann, Peter. J. Chem. Educ.2000, 77, 1056.

Atomic Properties / Structure |

Periodicity / Periodic Table |

Quantum Chemistry |

Theoretical Chemistry

The Genius of Slater's RulesJames L. ReedWith only a few modifications a procedure has been developed that yields the one-electron energies for atoms and ions with a level of detail very well suited for instruction in the structure and properties of atoms. It provides for the computation of very reasonable values for such properties as ionization energies, electron affinities, promotion energies, electronic transitions, and even XPS and ESCA spectra. Reed, James L. J. Chem. Educ.1999, 76, 802.

Atomic Properties / Structure |

Quantum Chemistry |

Theoretical Chemistry |

Spectroscopy

Chemistry of the Heaviest Elements-One Atom at a TimeDarleane C. Hoffman and Diana M. LeeA 75-year perspective of the chemistry of the heaviest elements, including a 50-year retrospective view of past developments, a summary of current research achievements and applications, and some predictions about exciting, new developments that might be envisioned within the next 25 years.Hoffman, Darleane C.; Lee, Diana M. J. Chem. Educ.1999, 76, 331.

Chromatography |

Instrumental Methods |

Isotopes |

Nuclear / Radiochemistry |

Separation Science |

Descriptive Chemistry |

Enrichment / Review Materials |

Atomic Properties / Structure

Experimental 4s and 3d Energies in Atomic Ground StatesJames L. BillsA new definition is given for the effective charge Zf. HF orbital energies e4s and e3d are used in concert with I4s and I3d to answer four questions: Why does the 4s sublevel fill before 3d? Why is ionization easier for 4s than 3d? When 4s23dn has e3d < e4s, why doesn't 4s23dn -> 4s13dn+1? Why are Cr and Cu each 4s13dn+1 instead of 4s23dn? Bills, James L. J. Chem. Educ.1998, 75, 589.

Atomic Properties / Structure

Electron Affinities of the Alkaline Earth Metals and the Sign Convention for Electron AffinityJohn C. WheelerIt has been known since 1987, both theoretically and experimentally, that the ion Ca- is stable. It is now certain that Sr-, Ba-, and Ra- are also stable, and accurate values for the electron affinities of Ca-, Sr-, and Ba- have been determined. Recommended values for these electron affinities, in the units commonly employed in introductory texts and with the sign convention used here, are 2.37, 5.03, and 13.95 kJ/mol for Ca, Sr, and Ba, respectively. Wheeler, John C. J. Chem. Educ.1997, 74, 123.

Moseley's Work on X-Rays and Atomic NumberC. W. HaighExplanation of the relationship between Moseley's work in determining atomic numbers, the spectrum of the hydrogen atom, the Bohr theory, and Slater's rules for screening constants.Haigh, C. W. J. Chem. Educ.1995, 72, 1012.

Simple Inorganic Substances: A New Approach (Sanderson, R.T.)Kauffman, Goerge B.This book stresses the cause-and-effect relationship between the structures of atoms and the properties of their compounds, with an emphasis on providing a thorough understanding of the most familiar and important inorganic compounds.Kauffman, Goerge B. J. Chem. Educ.1990, 67, A26.

Atomic Properties / Structure |

Descriptive Chemistry

Electron dormitory: AnalogueMorreale, CharlesAnalogous reasoning and relating filling a dormitory with people and an atom with electrons.Morreale, Charles J. Chem. Educ.1990, 67, 862.

Understanding electron configurations Rieck, David F.The author has successfully employed an analogy for understanding electron configurations recommended for use in secondary schools as well as in nonmajor sections of college general chemistry.Rieck, David F. J. Chem. Educ.1990, 67, 398.

Atomic Properties / Structure |

Nonmajor Courses

The periodicity of electron affinityMyers, R. ThomasIn general, the values of electron affinity for the elements can be understood in terms of their ground state electron configuration, and the screening (effective nuclear charge) exerted on the added electron by the electrons already present in the neutral atom.Myers, R. Thomas J. Chem. Educ.1990, 67, 307.

Visualization of electron clouds in atoms and moleculesDouglas, John E.110. Visualization of the electron orbital concept continues to challenge and intrigue chemical educators. [October and November 1989 Computer Series both inadvertently called number 107. Numbering restored by skipping 109 and calling January 1990 number 110.]Douglas, John E. J. Chem. Educ.1990, 67, 42.

Atomic Properties / Structure |

Molecular Properties / Structure

Teaching the shapes of the hydrogenlike and hybrid atomic orbitalsAllendoerfer, Robert D.The purpose of this article to show that, in this age of computer graphics, the "difficult to obtain" argument no longer has merit and to give an example of where the standard treatment gives insufficient attention to detail in describing the nodal surfaces of hybrid orbitals.Allendoerfer, Robert D. J. Chem. Educ.1990, 67, 37.

Principles of electronegativity Part I. General natureSanderson, R. T.The concept of electronegativity has been modified, expanded, and debated. The concept can be used to help students gain valuable insights and understanding of the cause-and-effect relationship between atomic structure and compound properties. This is the first in a series of articles that explores the important concept of electronegativity.Sanderson, R. T. J. Chem. Educ.1988, 65, 112.

Electrochemistry |

Periodicity / Periodic Table |

Noncovalent Interactions |

Atomic Properties / Structure |

Physical Properties |

Enrichment / Review Materials

Periodic contractions among the elements: Or, on being the right sizeMason, JoanContraction across the row, irregularities in the build up of the periodic table, the second row anomaly relativistic contraction and expansion among the heavier elements, post-transition anomaly, periodicities of physicochemical properties.Mason, Joan J. Chem. Educ.1988, 65, 17.

Interpretation of oxidation-reductionGoodstein, Madeline P.Presents an interpretation of the oxidation number system based upon the electronegativity principle, thus removing the adjective "arbitrary" frequently found in the descriptions of oxidation number.Goodstein, Madeline P. J. Chem. Educ.1970, 47, 452.

Oxidation / Reduction |

Oxidation State |

Atomic Properties / Structure |

Reactions

Role of f electrons in chemical bindingJohnson, O.Data presented suggests that f electrons, by their ineffective screening of the nuclear charge, exert an indirect effect on the binding strength of actions.Johnson, O. J. Chem. Educ.1970, 47, 431.

Atomic orbitals: Limitations and variationsCohen, Irwin; Bustard, ThomasThe three most widely used methods of arriving at a set of atomic orbitals afford respective hydrogen-like orbitals, self-consistent field orbitals, and various analytical approximations such as the Slater or Morse orbitals, all of which may differ greatly in shape and size from each other.Cohen, Irwin; Bustard, Thomas J. Chem. Educ.1966, 43, 187.

Atomic Properties / Structure |

Quantum Chemistry

General chemistry exercise using atomic and molecular orbital modelsWalker, Ruth A.Styrofoam balls and pipecleaners are used to construct models designed to convey an understanding of the three-dimensionality of the electron distribution in the ground state atom and the effect of bonding on this distribution.Walker, Ruth A. J. Chem. Educ.1965, 42, 672.

Atomic Properties / Structure |

Molecular Modeling |

Molecular Properties / Structure |

Covalent Bonding

LettersGates, Henry S.Brings the reader's attention to work done by Petit and Dulong in revising a large number of atomic weights in order to bring all of their reported atomic heat capacities into agreement with the hypothesis that atomic heat capacity is the same for all elements.Gates, Henry S. J. Chem. Educ.1964, 41, 575.

The principle of minimum bending of orbitalsStewart, George H.; Eyring, HenryThe authors present a theory of valency that accounts for a variety of organic and inorganic structures in a clear and easily understood manner.Stewart, George H.; Eyring, Henry J. Chem. Educ.1958, 35, 550.

A new periodic table based on the energy sequence of atomic orbitalsWalker, W. R.; Curthoys, G. C.Since the theory of atomic and molecular orbitals has proven to be of such value in interpreting the data of inorganic chemistry, it is hoped that a new periodic table based on the energy sequence of atomic orbitals will be an aid to the further systematizing of chemical knowledge.Walker, W. R.; Curthoys, G. C. J. Chem. Educ.1956, 33, 69.

Atomic structure and the photoelectric effectBrockett, Clyde P.The ubiquitous and inexpensive 110-volt, 2-watt neon glow lamp appears to have been overlooked as a device well suited to a brief but telling demonstration of a few key principles of atomic structure that underlie the study of electrovalence and comparative chemistry.Brockett, Clyde P. J. Chem. Educ.1953, 30, 498.